Question

4) Which of the following set of quantum number is not possible?
(A) n=3, l=2, m=-1, s=-1/2
(B) n=4, l=2, m=-2, s=+1/2
(C) n=3, l=1, m=2, s=-1/2
(D) n=4, l=1, m=1, s=+1/2

Answer 1

(a) The given set of quantum numbers is not possible because the value of the principal quantum number (n) cannot be zero.
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Answer 2

Set (C) is not a possible set of quantum numbers, while set (A), set (B), and set (D) are possible sets.

Quantum numbers are used to describe the unique state of an electron in an atom. There are four quantum numbers, n, l, m, and s, each with specific allowed values.

(A) n=3, l=2, m=-1, s=-1/2: This set of quantum numbers is possible, as n can take values from 1 to infinity, l can take values from 0 to n-1, m can take values from -l to l, and s can take values of ±1/2.

(B) n=4, l=2, m=-2, s=+1/2: This set of quantum numbers is possible.

(C) n=3, l=1, m=2, s=-1/2: This set of quantum numbers is not possible, as m can take values from -l to l, and in this case, m=2 is outside the allowed range for l=1.

(D) n=4, l=1, m=1, s=+1/2: This set of quantum numbers is possible, as all values are within the allowed range.

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